You are given a recipe for a buffer that contains 8% (w/v) CaCl2.2H2O, however, you only have CaCl2 anhydrous available to you. How much CaCl2 anhydrous do you need to make 3.5 L of the buffer with the same molar concentration as in the recipe? Show your calculations.
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You are given a recipe for a buffer that contains 8% (w/v) CaCl2.2H2O, however, you only
have CaCl2 anhydrous available to you.
How much CaCl2 anhydrous do you need to make 3.5 L of the buffer with the same molar
concentration as in the recipe? Show your calculations.
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- Consider the titration of butyric acid (HBut) with sodium hydroxide. In an experiment, 50.00 mL of 0.350 M butyric acid is titrated with 0.225 M NaOH. Ka HBut=1.5105. (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of sodium hydroxide is required to reach the equivalence point? (d) What is the pH of the solution before any NaOH is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?Which of these buffers involving a weak acid HA has the greater resistance to change in pH? Explain your answer. (i) [HA] =0.100 M = [A] (ii) [HA] = 0.300 M = [A]Two buffers are prepared by adding an equal number of moles of formic acid (HCOOH) and sodium formate (HCOONa) to enough water to make 1.00 LL of solution. Buffer A is prepared using 1.00 molmol each of formic acid and sodium formate. Buffer B is prepared by using 0.010 molmol of each. (Ka(HCOOH)=1.8×10−4.) Calculate the pHpH of each buffer. Which buffer will have the greater buffer capacity?
- A buffer is prepared by adding 2.50g of lithium fluoride to 125 mL of 0.648M hydrofluoric acid. You may assume there is no change in volume after the substances are mixed. 1. What is the pH of this buffer? 2. Write the equation by which this buffer would react to a strong acid. 3. If 50.0 mL of 0.0750M nitric acid is added to the original buffer, what would be the pH? 4. Write the equation by which this buffer would react to the addition of a strong base. 5. You add 75.0 mL of 0.900M potassium hydroxide to this buffer. Assuming no change in volume, what would be the pH after this addition? 6. You add 450 mL of a 0.27M hydrochloric acid solution to the original buffer. What is the pH of the resulting solution?A buffer is prepared by adding 0.40 moles of formic acid (HCOOH) and 0.60 moles of sodium formate (HCOONa) to enough water to make 1.00 L of solution. a. Calculate the pH of this buffer. b. How many moles of HCOONa must be added to 1.0 L of a 0.40M HCOOH solution to prepare a buffer with pH 4.24? c. Calculate the change in pH for 100mL of the buffers from part a) and b) upon the addition of 5.00 mL of 1.00M HCl.You wish to prepare a buffer consisting of acetic acid and sodium acetate with a total acetic acid plus acetate concentration of 250 mM and a pH of 5.0. What concentrations of acetic acid and sodium acetate should you use? Assuming you wish to make 2 liters of this buffer, how many moles of acetic acid and sodium acetate will you need? How many grams of each will you need (molecular weights: acetic acid 60.05 g mol^-1, sodium acetate, 82.03 g mol^-1)?
- A solution with the volume of one liter contains 0.5 mole HC2H3O2, 0.5 mole C2H3O2- ion, and 0.5 mole Na+ Ka for HC2H3O2 is 1.8 x 10-5. What is the pH of the solution? Is the solution a buffer? Why or why not? Write down the net ionic equation for the reaction which occurs if a little H+ ion is added to the solution.A buffer is made using 100.0 mL of 0.100 M CH_{3}3CH_{2}2COOH (propanoic acid) and 100.0 mL of 0.100 M NaCH_{3}3CH_{2}2COO (sodium propanoate). A) Explain in your own words what will occur (at the molecular level) when an nitric acid is added to the buffer? What would be the effect on the pH? B) Explain in your own words what will occur when LiOH is added tot he buffer? What would be the effect on the [H+]?2. You wish to prepare a buffer containing acetic acid and sodium acetate with a total acetic acid and acetate concentration of 450 mM and a pH of 5.5 (a) What are the final concentrations of acetic acid and sodium acetate in the buffer? (b) Calculate the number of moles of acetic acid and sodium acetate that you would need to make 1.5 L of the buffer. (c) How many grams of acetic acid and sodium acetate would you need to make 1.5 L of the buffer (molecular weight of acetic acid=60.05 g/mol: molecular weight of sodium acetate =82.03 g/mol)?
- A buffer solution contains 0.275 M of acetic acid, HC2 H 3 O 2 , and 0.350 M of its conjugate salt, KC 2 H 3 O 2 .i) Write the balanced chemical equation for reaction between the appropriate buffer component ( HC 2 H 3 O 2 or KC 2 H 3 O 2 ) and H 3 O + ions from a strong acid (to show how the buffer works). ii) Calculate the pH after 0.0500 mol of HCl is added to 1.00 L of the buffer solution? K a (HC 2 H 3 O 2 ) = 1.8 × 10 -5You are tasked with making a buffer solution containing equal amounts of propionic acid from a 99.5 wt% solution (d = 0.993 g/mL, FW = 74.08 g/mol) and sodium propionate (solid, FW = 96.06 g/mol). What concentration of the buffer must be prepared to prevent a change in the pH by more than 0.5 pH units after the addition of 10.00 mL of 3.00 M HCl to 100.0 mL of the buffer solution? The Ka for propionic acid is 1.76 x 10-5.A. What is the pH of a buffer prepared by adding 0.405 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7. B. What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base.
